The degree of dissociation of `Ca(NO_3)_2` in a dilute aqueous solution, containing 7.0g of salt per 100 g of water at 100° C is 70%. It the vapour pressure of water at 100°C is 760 mm Hg, calculate the vapour pressure of the solution.

What is the vapour pressure of pure water at 100^(@)C temperature ?

6.0 g of urea (molecular weight=60) was dissolved in 9.9 moles of water. If the vapour pressure of pure water is P^@ , the vapour pressure of solution is :

Calculate the molality of an aqueous solution containing 3.0g of urea (mol.mass=60) in 250g of water.

2 g of O-2 at 0^@C and 760 mm of Hg pressure has volume

At 25^(@) C temperature, vapour pressure of water is 23.55mm. What will be the vapour pressure of the solution when 6g of urea is mixed with 100g of water?

At 25^(@) C temperature, vapour pressure of water is 23.55mm. What will be the vapour pressure of the solution when 6g of urea is mixed with 100g of water?

Two liquids A and B form an ideal solution. At 300 k, the vapour pressure of a solution containing 1 mole of A and 3 moles of B is 550 mm of Hg. At the same temperature, if one mole of B is added to this solution, the vapour pressure of the solution increases by 10 mm of Hg. Determine the vapour pressure of A and B in their pure states.

Two liquids X and Y on mixing form an ideal solution. At 30^@C , the vapour pressure of the solution containing 3 mol of X and 1 mol of Y is 550 mm Hg. But when 4 mol of X and 1 mol of Y are mixed, the vapour pressure of the solution thus formed is 560 mm Hg. What would be the vapour pressure of pure X and Y at this temperature?

The degree of dissociation of water at 25^@C is 1.9xx10^-7% and density is 1g cm cube. The ionic constant for water is